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- a) What would you expect the magnitude and sign of ΔHSOLUTE, ΔHSOLVENT, and ΔHMIXING to be for CH2Cl2 as solute and acetone as solvent? Circle your choices below. Then, fill in the most important IM force that exists between solute molecules, between solvent molecules and between solute and solvent molecules. b) Based on this, what is the overall enthalpy change (HSOLUTION) for dissolving CH2Cl2 in acetone expected to be? (negative/positive/ near zero). Would you expect CH2Cl2 to dissolve in acetone? (yes/no). Explain your answers to both of the questions above. Consider the energy and entropyExtra information: freezing point depression constant for the solvent (20.0 degrees Celcius kg/mol for cyclohexane)Boiling Point Elevation/Freezing Point Depression T = m K where, for freezing point depression: T = T(pure solvent) - T(solution) and for boiling point elevation: T = T(solution) - T(pure solvent) m = (# moles solute / Kg solvent) Kb = boiling point elevation constant. Kf = freezing point depression constant. Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow. Solvent Formula Kb(°C / m) Kf(°C / m) Water H2O 0.512 1.86 Ethanol CH3CH2OH 1.22 1.99 Chloroform CHCl3 3.67 Benzene C6H6 2.53 5.12 Diethyl ether CH3CH2OCH2CH3 2.02
- Assuming that pentane and hexane form an ideal solution, A. Calculate the amount of pentane to be added to 65.0 g of hexane to obtain a minimum dG of mixing from mixing those two components. [MM pentane; 72.15, MM hexane; -86.18] B. Calculate the dS of mixing the components of the mixture above.Please indicate true (T) or false (F) as appropriate: Justify I) The vapor pressure of a solvent is reduced by the presence of a non-volatile solute II) In an ideal solution, the vapor pressure is increased by the presence of a solute Volatile. III) Sea water freezes at a lower temperature than sugar water. IV) In the laboratory, chemists use this effect to judge the purity of a component solid: if impurities are present, the freezing point of the compound is lower than the accepted value. A) TFTF B) TTFT C) FTFF D) TTTTThe solvent for an organic reaction is prepared by mixing 70.0 mL of acetone (C3H6OC3H6O) with 56.0 mL of ethyl acetate (C4H8O2C4H8O2). This mixture is stored at 25.0 ∘C∘C. The vapor pressure and the densities for the two pure components at 25.0 ∘C∘C are given in the following table. What is the vapor pressure of the stored mixture? Compound Vapor pressure(mmHg) Density(g/mLg/mL) acetone 230.0 0.791 ethyl acetate 95.38 0.900
- 1. Suppose each pair below is mixed well. What comes out as the simplest example of liquid mixing?A. 12 M sulfuric acid solution and 12 M sodium hydroxide solutionB. water with 80% ethanolC. ethane with methaneD. acetic acid and waterDraw and label completely the liquid-vapor phase diagram of the acetone chloroform system given the following data. a) Only one liquid phase existsb) There is an azeotrope at 64.0 mole% chloroform with taze = 64.4 oC.c) Pure acetone and chloroform boil at 56.1 and 61.2 oC respectively.When pure furfural (solvent) is added to a mixture containing 0.2 mass fraction diphenylhexane and 0.8 mass fraction docosane, two separate layers can be obtained. If the composition of the two layers are as shown in the table, how much solvent was added to 500 kg of solution of docosane and diphenylhexane?
- 1. What is the mole percent of methanol in your starting solution (composed of 1.5 mL and 6 mL isopropanol)? 2. Using the vapor-liquid equilibrium data graph (NOTE: You have to make this graph using the data provided) and your answer from question 1, answer the following: If your first distillate was 49 mole percent methanol, how many theoretical plates were in your distillation setup? Data Mole % of Methanol Temperature (°C) Vapor Liquid 66.22 95.35 90.10 67.94 89.10 79.00 70.22 80.00 66.05 72.67 68.50 52.20 74.78 57.00 40.80 77.06 42.85 29.30 78.94 29.00 19.50 81.00 13.20 8.10It is desired to prepare 2.5 m^3 of a 60 mol percent methanol - water solution. Determine the volumes of methanol and water required to be mixed at ambient temperature given that the partial molar volumes of methanol and water are 58.3x10^-6m^3/mol and 17.2 x 10 m^3/mol respectively. The density of the methanol is 782.51 kg/m^3. Do not use chatgpt. Thank you!If the mixing ratio of CO2 is 350ppmv calculate the CO2 concentration in terms of moles/L and molecules/cm3 . What is the partial pressure of CO2?